Final answer:
F₂ likely has the weakest dispersion forces compared to Cl₂, Br₂, and I₂, as it is the smallest and lightest molecule with fewer electrons for temporary polarization.Hence, option C is the correct answer.
Step-by-step explanation:
The molecule most likely to have the weakest induced dipole-induced dipole interaction among Cl₂, Br₂, F₂, and I₂ is F₂. This is because induced dipole-induced dipole interactions, also known as London dispersion forces, become stronger with increasing molecular size and mass. Larger and heavier atoms and molecules have more electrons that can become momentarily polarized, thus leading to stronger temporary dipoles. F₂ is the smallest and lightest of the halogens mentioned, with the least amount of electrons available for dispersion forces. In contrast, I₂ has the strongest dispersion forces due to its larger molecular size and higher electron count. Therefore, compounds like F₂ are gases at room temperature, indicating weaker attractive forces, while I₂ is solid, reflecting stronger attractive forces.